1. The Periodic
Table

2. Classification of Elements

3. Metals, Nonmetals, and Metalloids

4. Horizontal rows are called periods There are 7 periods1 2 3 4 5 6 7

5. The 18 vertical columns are called families or groups.
Elements are placed in columns by similar properties.

6. Group Numbers on the Periodic Table

7. Group Names Halogens Noble Gases Chalcogens Alkali Metals
Alkaline Earth Metals
Lanthanides
Actinides

8. Solid, Liquid, and Gaseous Elements

9. Periodic Trends

10. Periodic Trends
Atomic radius: the distance from the center of an atom's nucleus to its outermost electron.
Since the electron cloud does not have an exact boundary, the atomic radius is usually measured by finding the distance between the centers of two atoms.

11. Atomic Radius
Atomic Radius
Increases to the LEFT and DOWN

12. Periodic Trends
Ionic Size: Atoms gain or lose electrons to gain noble gas configurations, or pseudonoble gas configurations.
Metals lose outer electrons forming cations which are smaller than the atoms they were made from.
Nonmetals gain outer electrons forming anions which are larger than the atoms they were made from.

13. Ionic Radius Ionic Radius Cations (+) smaller Anions (–) larger
lose e-
smaller
© 2002 Prentice-Hall, Inc.
Anions (–)
gain e
larger

14. Periodic Trends
Ionization energy: the energy required to remove an electron from a gaseous atom or ion.
Removing one electron makes a +1 ion.
The energy required is called the first ionization energy.

15. Ionization Energy
Ionization Energy
Increases UP and to the RIGHT

16. Periodic Trends
Electron Affinity: a measure of an atom's attraction, or affinity, for an extra electron.

17. Periodic Trends
Atoms that have a greater attraction for an added electron have a more negative electron affinity.
The higher the electron affinity, the higher the negative value. Nonmetals, other than the noble gases, have the greatest electron affinities.

18. Electron Affinity:
Electron affinity generally decreases down a group since the attraction by the nucleus on the outer level electron is weakened by the increase in atomic size.
Electron affinity generally increases across a period because the atoms become smaller and the nuclear charge increases.

19. Periodic Trends Activity: refers to the tendency of an atom to react.
Activity increases toward the lower left side of the periodic table, for metals.
Activity increases toward the upper right corner of the periodic table, except the noble gases, for nonmetals.
Fluorine is the most active element. It reacts with everything except He, Ne, and Ar.
Noble gases are generally very unreactive.

21. STOP Presentation Pass out Periodic Trends worksheet to the students.
Please read the instructions at the top of worksheet.
Once students have had time to complete the worksheet, please continue to show this presentation for the answers. 

22. Answers: Trends from the Periodic Table

23. #1 What do you expect the following atoms to do when bonding with other atoms?

24. Bonding Atom Reason Calcium is a metal Fluorine is a nonmetal
Calcium-A-Lose electrons
Fluorine-B-Gain electrons
Neon-C- Neither lose or gain electrons
Argon-C-Neither lose or gain electrons
Oxygen-B-Gain electrons
Calcium is a metal
Fluorine is a nonmetal
Neon is a noble gas
Argon is a noble gas
Oxygen is a nonmetal

25. Bonding Atom Reason 6. Zinc is a metal 7. Lithium is a metal
6. Zinc-A-Lose electrons
7. Lithium-A-Lose electrons
8. Sulfur-B-Gain electrons
9. Helium-C-Neither lose or gain electrons
10. Sodium-A-Lose electrons
6. Zinc is a metal
7. Lithium is a metal
8. Sulfur is a nonmetal
9. Helium is a noble gas
10. Sodium is a metal

26. #2 Predict the ions formed by the following elements

27. Ion formation Reason Aluminum, Al +3
1. Aluminum is a metal-which means it loses electrons. It is in Group IIIA (look at the top of the column in which Aluminum is under) It has 3 valence electrons. It needs to lose three electrons in order to have the valence electrons of the noble gas Neon (which has 8 valence electrons). Because it loses 3 electrons it the ion is positively charged.
Aluminum, Al +3

28. Ion Formation Reason 2. Phosphorus, P -3
2. Phosphorus is a nonmetal-which mean it gains electrons. It is in Group VA. It has 5 valence electrons; therefore it needs 3 more electrons in order to have the valence electrons of the noble gas Neon (which has 8 valence electrons). It is -3 because electrons are negatively charged.

29. Ion Formation Reason 3. Nitrogen, N -3
3. Nitrogen is a nonmetal-which mean it gains electrons. It is in Group VA. It has 5 valence electrons; therefore it needs 3 more electrons in order to have the valence electrons of the noble gas Neon (which has 8 valence electrons). It is -3 because electrons are negatively charged.

30. Ion Formation Reason 4. Lead, Pb +4
4. Lead is a metal-which means it loses electrons. It is in Group IVA. It has 4 valence electrons. It needs to lose four electrons in order to have the valence electrons of the noble gas Xeon (which has 8 valence electrons). Because it loses 4 electrons, the ion is positively charged.

31. #3 Predict the number of valence electrons the following atoms.

32. Valence Number Reason Tin, Sn 4 Bismuth, Bi 5
Tin is a member of group IVA. Which means it has 4 valence electrons
Bismuth is a member of group VA. Which means it has 5 valence electrons.

33. Valence Number Reason Silicon, Si 4 Strontium, Sr 2
3. Silicon is a member of IVA. Which means it has 4 valence electrons.
4. Strontium is a member of IIA. Which means it has 2 valence electrons.

34. Predict the following electron configuration
4. Aluminum: 1s22s22p63s23p1
5. Bromine: 1s22s22p63s23p64s23d104p5

35. Prediction for new element, atomic number 114
6. Metal: Since it would be in the same column as Lead-which is a metal. It would lose electrons, be a good conductor of heat and electricity, have luster, be ductile and malleable.
7. The number of valence electrons for the new element 114 is 4 valence electrons, because it would be in column IV-which has 4 valence electrons.
8. The ion formation of the new element 114 is +4.

36. A new element, atomic number 118, was discovered.
9. Predict some properties of this element.
It would be a noble gas, be relatively unreactive, have 8 valence electrons, form no ions.